Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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Multiple Choice

Which of the following is the correct Lewis dot structure for the neutral compound CF2O?

The central carbon atom is single-bonded to oxygen and single-bonded to each fluorine; oxygen has two lone pairs.

The central carbon atom is triple-bonded to oxygen and single-bonded to each fluorine; oxygen has one lone pair.

The central carbon atom is single-bonded to oxygen and double-bonded to each fluorine; oxygen has three lone pairs.

The central carbon atom is double-bonded to oxygen and single-bonded to each fluorine; all atoms have complete octets.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons in CF2O. Carbon has 4 valence electrons, each fluorine has 7, and oxygen has 6. Add these together to find the total electrons available for bonding and lone pairs.

Step 2: Identify the central atom, which is carbon in this case, because it is less electronegative than oxygen and fluorine and can form multiple bonds.

Step 3: Connect the central carbon atom to the two fluorine atoms and the oxygen atom with single bonds initially. This uses 6 electrons (3 bonds × 2 electrons each).

Step 4: Complete the octets of the fluorine atoms by adding three lone pairs (6 electrons) to each fluorine, since fluorine typically forms only one bond and has three lone pairs.

Step 5: Use the remaining electrons to complete the octet on oxygen. If oxygen does not have a full octet with a single bond, form a double bond between carbon and oxygen. Adjust lone pairs accordingly so that all atoms have complete octets.